Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a net ionic equation for the reaction between sodium thiosulfate and iodine. It begins with balancing the molecular equation, followed by determining the states of each compound. The tutorial then demonstrates how to split strong electrolytes into ions to form the complete ionic equation, and finally, how to derive the net ionic equation by removing spectator ions. The video concludes by ensuring that both charge and atoms are balanced in the final equation.

What is the first step in writing a net ionic equation?

• Determine the states of substances

• Identify spectator ions

• Split compounds into ions

• Balance the molecular equation

How do you balance the number of sodium atoms in the equation?

• Adjust the coefficients

• Add more iodine

• Double the sodium thiosulfate

• Remove excess sodium

What is the state of sodium compounds in the reaction?

• Liquid

• Gas

• Solid

• Aqueous

Why is iodine not split into ions in the net ionic equation?

• It is a molecular substance

• It is insoluble

• It reacts with sodium

• It is a gas

What is the purpose of identifying spectator ions?

• To balance the equation

• To simplify the net ionic equation

• To find the limiting reactant

• To determine solubility

Which ions are considered spectator ions in this reaction?

• Sulfate ions

• Sodium ions

• Iodine ions

• Thiosulfate ions

What ensures the charge is balanced in the net ionic equation?

• Conservation of charge

• Equal number of atoms

• Equal number of ions

• Conservation of mass

What is the final step in writing the net ionic equation?

• Ensuring charge balance

• Crossing out spectator ions

• Writing the states

• Balancing atoms

What is the charge on the thiosulfate ion in the net ionic equation?

• 1-

• 2-

• 3-

• 4-

What is the significance of balancing atoms in the net ionic equation?

• To determine the reaction rate

• To identify the limiting reactant

• To maintain the law of conservation of mass

• To ensure the reaction is complete